Determining the Order of a Chemical Reaction

In an aqueous solution, glucose decomposed according to the results shown below.
(a) Demonstrate that the reaction is first order.
(b) Calculate the rate constant for the decomposition process.
(c) Calculate the half-life (t1/2) for glucose under the specified conditions.

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For the second order reaction below, the initial concentration of A is 1.34M. If k=7.61x10(exponent negative 4) seconds(exponent negative 1), what is the concentration of A after 18.3 minutes?
2A-->B rate=k[A](exponent2)

Please show all work and keep things as simple as possible in the following three problems on chemistry and its rate mechanisms.
The Rate Law.
1) A possible mechanism for thereaction between H2 and CO is shown below, where RDS is the rate-determining step. What is the rate law for the overall reaction?
H2 ? 2 H

See the attached file.
1. Now consider the following reaction and data:
H 2 +2BrCl→2HCl+Br 2
Time (s)
Br 2 concentration (M)
5 1.35
15 1.65
Part A
What is the average rate of formation of Br 2 ?Express your answer to three decimal places and include the appropriate units.
2. Consider thereaction: A(g)+1 2 B(

If the overall reaction is the sum of theorder of the reagents, and:
Zero order = changing concentration of the reactant does not affect thereaction rate.
First order = doubling the concentration of any reactant doubles thereaction rate
Second order = doubling the concentration of any reactant quadruples thereaction

A reaction is defined by the following scheme:
X à Y
When the concentration of X in a solution is 1.02 M, the half-life (t1/2) is 160 seconds.
When the concentration of X in solution is 2.05 M, the half-life (t1/2) is 80 seconds.
The above information applies when thereaction takes place at 25 degrees Celsius.